Mass in grams of copper deposited by passing $9.6487 \ A$ current through a voltmeter containing copper sulphate solution for $100 \ s$ is (Given : Molar mass of $Cu: 63 \ g \ mol^{-1}, 1 \ F=96487 \ C$ ) (in $g$)

$A$ metal plate of dimension $(1 \times 2 \ cm^2)$ has to be coated on both sides by $Cu$ metal. How long does it take to deposit $Cu$ of $0.01 \ cm$ thickness,if $1.5 \ A$ current is used (in $s$)? [Electrochemical equivalence of $Cu$ is $0.0003 \ g/C$ and the density of $Cu$ is $9 \ g/cm^3$]

The mass of zinc produced by the electrolysis of zinc sulphate solution with a steady current of $0.015 \ A$ for $15$ minutes is . . . . . . $ \times 10^{-4} \ g$. (Atomic mass of zinc $= 65.4 \ amu$)

Match the column :-

Column $I$ (Reduction process)	Column $II$ (Charge required)
$(a)$ $1$ mol of $MnO_4^-$ to $Mn^{2+}$	$(p)$ $193000$ $C$
$(b)$ $1$ mole of $Cr_2O_7^{2-}$ to $Cr^{3+}$	$(q)$ $289500$ $C$
$(c)$ $1$ mole of $Sn^{4+}$ to $Sn^{2+}$	$(r)$ $482500$ $C$
$(d)$ $1$ mole of $Al^{3+}$ to $Al$	$(s)$ $579000$ $C$

When an electric current is passed through acidulated water,$112 \ mL$ of hydrogen gas at $N.T.P.$ collects at the cathode in $965 \ seconds$. The current passed,in amperes,is:

$A$ current is passed for $2 \, \text{hours}$ through an acidic solution,liberating $11.2 \, L$ of oxygen at $NTP$ at the anode. What will be the amount of copper deposited at the cathode by the same current when passed through a solution of copper sulphate for the same duration? .......... $g$